General Chemistry II Comprehensive
Final Exam Study guide With 100%
Verified Solutions
Ionic CORRECT ANSWERS Intermolecular forces: ion-ion forces
Properties: brittle, hard, high-melting
Examples: NaCl, KBr, MgCl2
Molecular CORRECT ANSWERS Intermolecular forces: dispersion forces, dipole-dipole
forces, hydrogen bonds
Properties: soft, low-melting, nonconducting
Examples: H2O, Br2, CO2, CH4
Covalent network CORRECT ANSWERS Intermolecular forces: covalent bonds
Properties: hard, high-melting
Examples: C (diamond), SiO2
Metallic CORRECT ANSWERS Intermolecular forces: metallic bonds
Properties: variable hardness and melting point, conducting
Examples: Na, Zn, Cu, Fe
Simple cubic CORRECT ANSWERS Stacking pattern: a-a-a-a
Coordination number: 6
Space used (%): 52
Unit cell: primitive-cubic
Body-centered cubic CORRECT ANSWERS Stacking pattern: a-b-a-b
Coordination number: 8
Space used (%): 68
Unit cell: body-centered cubic
Hexagonal closest-packing CORRECT ANSWERS Stacking pattern: a-b-a-b
Coordination number: 12
Space used (%): 74
Unit cell: (noncubic)
Cubic closest-packing CORRECT ANSWERS Stacking pattern: a-b-c-a-b-c
Coordination number: 12
Space used (%): 74
Unit cell: face-centered cubic
Molarity (M) CORRECT ANSWERS Moles of solute/liters of solution
,Mole faction (X) CORRECT ANSWERS Moles of component/Total moles making up the
solution
Mass percent CORRECT ANSWERS (Mass of component/total mass of solution) x
100%
Parts per million (ppm) CORRECT ANSWERS (Mass of component/total mass of
solution) x10^6
Parts per billion (ppb) CORRECT ANSWERS (Mass of component/total mass of
solution) x10^9
Molality (m) CORRECT ANSWERS Moles of solute/mass of solvent (kg)
Molarity (M) CORRECT ANSWERS Units: mole solute/L solution
Advantages: useful in stoichiometry, by volumes
Disadvantages: temperature-dependent, must know density to find solvent mass
Mole fraction (X) CORRECT ANSWERS Units: none
Advantages: temperature-independent, useful in special applications
Disadvantages: measure by mass, must know density to convert to molarity
Mass % CORRECT ANSWERS Units: %
Advantages: temperature-independent, useful in small amounts
Disadvantages: measure by mass, must know density to convert to molarity
Molality (m) CORRECT ANSWERS Units:
Advantages: temperature-independent, useful in special applications
Disadvantages: measure by mass, must know density to convert to molarity
Henry's Law CORRECT ANSWERS Solubility = kp
Colligative properties CORRECT ANSWERS In comparing the properties of a pure
solvent with those of a solution:
- the vapor pressure of the solution is lower
- the boiling point of the solution is higher
- the freezing (or melting) point of the solution is lower
- the solution gives rise to osmosis, the migration of solvent molescules through a
semipermeable membrane
Van't Hoff factor CORRECT ANSWERS i = moles of particle in solution/moles of solute
dissolved
Integrated rate law for a zeroth-order reaction CORRECT ANSWERS [A]t = -kt + [A]0
K= -(slope)
, Integrated rate law for a first-order reaction CORRECT ANSWERS ln ([A]t/[A]0) = -kt
K= -(slope)
Integrated rate law for a second-order reaction CORRECT ANSWERS 1/[A]t = kt +
1/[A]0
K= slope
A compound is soluble if it contains one of the following cations CORRECT ANSWERS
Li+, Na+, K+, Rb+, and Cs+ (Group 1A cations)
NH4+ <—- ammonium cation
A compound is soluble if it contains one of the following anions CORRECT ANSWERS
Cl-, Br-, I- (halide anions) except Ag+, Hg22+, and Pb2+ halides.
No3-, ClO4-, Acetate, So4- except
Sr2+, Ba2+, Hg22+, and Pb2+ sulfates
What is the pH at the equivalence point of a weak acid-strong base titration? CORRECT
ANSWERS pH>7, basic solution
What is the pH at the equivalence point of a Strong acid-strong base titration?
CORRECT ANSWERS pH=7, neutral solution
What is the pH at the equivalence point of a Strong acid-weak base titration?
CORRECT ANSWERS pH<7, acidic solution
Kn equals CORRECT ANSWERS 1/[H30+][OH-]
pH at first equivalence point CORRECT ANSWERS pKa1+pka2/2
If the initial ion product is greater than Ksp then what will happen? CORRECT
ANSWERS An ionic compound will precipitate
If the initial ion product is less than Ksp what will happen? CORRECT ANSWERS No
solid ionic product will precipitate.
If a solution goes up in temperature what is the sign for enthalpy? CORRECT
ANSWERS - delta H
If a solution goes down in temperature what is the sign for enthalpy? CORRECT
ANSWERS + delta H
Final Exam Study guide With 100%
Verified Solutions
Ionic CORRECT ANSWERS Intermolecular forces: ion-ion forces
Properties: brittle, hard, high-melting
Examples: NaCl, KBr, MgCl2
Molecular CORRECT ANSWERS Intermolecular forces: dispersion forces, dipole-dipole
forces, hydrogen bonds
Properties: soft, low-melting, nonconducting
Examples: H2O, Br2, CO2, CH4
Covalent network CORRECT ANSWERS Intermolecular forces: covalent bonds
Properties: hard, high-melting
Examples: C (diamond), SiO2
Metallic CORRECT ANSWERS Intermolecular forces: metallic bonds
Properties: variable hardness and melting point, conducting
Examples: Na, Zn, Cu, Fe
Simple cubic CORRECT ANSWERS Stacking pattern: a-a-a-a
Coordination number: 6
Space used (%): 52
Unit cell: primitive-cubic
Body-centered cubic CORRECT ANSWERS Stacking pattern: a-b-a-b
Coordination number: 8
Space used (%): 68
Unit cell: body-centered cubic
Hexagonal closest-packing CORRECT ANSWERS Stacking pattern: a-b-a-b
Coordination number: 12
Space used (%): 74
Unit cell: (noncubic)
Cubic closest-packing CORRECT ANSWERS Stacking pattern: a-b-c-a-b-c
Coordination number: 12
Space used (%): 74
Unit cell: face-centered cubic
Molarity (M) CORRECT ANSWERS Moles of solute/liters of solution
,Mole faction (X) CORRECT ANSWERS Moles of component/Total moles making up the
solution
Mass percent CORRECT ANSWERS (Mass of component/total mass of solution) x
100%
Parts per million (ppm) CORRECT ANSWERS (Mass of component/total mass of
solution) x10^6
Parts per billion (ppb) CORRECT ANSWERS (Mass of component/total mass of
solution) x10^9
Molality (m) CORRECT ANSWERS Moles of solute/mass of solvent (kg)
Molarity (M) CORRECT ANSWERS Units: mole solute/L solution
Advantages: useful in stoichiometry, by volumes
Disadvantages: temperature-dependent, must know density to find solvent mass
Mole fraction (X) CORRECT ANSWERS Units: none
Advantages: temperature-independent, useful in special applications
Disadvantages: measure by mass, must know density to convert to molarity
Mass % CORRECT ANSWERS Units: %
Advantages: temperature-independent, useful in small amounts
Disadvantages: measure by mass, must know density to convert to molarity
Molality (m) CORRECT ANSWERS Units:
Advantages: temperature-independent, useful in special applications
Disadvantages: measure by mass, must know density to convert to molarity
Henry's Law CORRECT ANSWERS Solubility = kp
Colligative properties CORRECT ANSWERS In comparing the properties of a pure
solvent with those of a solution:
- the vapor pressure of the solution is lower
- the boiling point of the solution is higher
- the freezing (or melting) point of the solution is lower
- the solution gives rise to osmosis, the migration of solvent molescules through a
semipermeable membrane
Van't Hoff factor CORRECT ANSWERS i = moles of particle in solution/moles of solute
dissolved
Integrated rate law for a zeroth-order reaction CORRECT ANSWERS [A]t = -kt + [A]0
K= -(slope)
, Integrated rate law for a first-order reaction CORRECT ANSWERS ln ([A]t/[A]0) = -kt
K= -(slope)
Integrated rate law for a second-order reaction CORRECT ANSWERS 1/[A]t = kt +
1/[A]0
K= slope
A compound is soluble if it contains one of the following cations CORRECT ANSWERS
Li+, Na+, K+, Rb+, and Cs+ (Group 1A cations)
NH4+ <—- ammonium cation
A compound is soluble if it contains one of the following anions CORRECT ANSWERS
Cl-, Br-, I- (halide anions) except Ag+, Hg22+, and Pb2+ halides.
No3-, ClO4-, Acetate, So4- except
Sr2+, Ba2+, Hg22+, and Pb2+ sulfates
What is the pH at the equivalence point of a weak acid-strong base titration? CORRECT
ANSWERS pH>7, basic solution
What is the pH at the equivalence point of a Strong acid-strong base titration?
CORRECT ANSWERS pH=7, neutral solution
What is the pH at the equivalence point of a Strong acid-weak base titration?
CORRECT ANSWERS pH<7, acidic solution
Kn equals CORRECT ANSWERS 1/[H30+][OH-]
pH at first equivalence point CORRECT ANSWERS pKa1+pka2/2
If the initial ion product is greater than Ksp then what will happen? CORRECT
ANSWERS An ionic compound will precipitate
If the initial ion product is less than Ksp what will happen? CORRECT ANSWERS No
solid ionic product will precipitate.
If a solution goes up in temperature what is the sign for enthalpy? CORRECT
ANSWERS - delta H
If a solution goes down in temperature what is the sign for enthalpy? CORRECT
ANSWERS + delta H
